QQuestionChemistry
QuestionChemistry
What is the empirical formula for a compound formed by fluorine and rubidium?
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Step 1:I'll solve this step by step using proper LaTeX formatting:
Step 2:: Determine the charges of the elements
- Rubidium (Rb) is in Group 1, so it has a charge of $$+1
- Fluorine (F) is in Group 17, so it has a charge of - 1
Step 3:: Determine the ratio of ions to balance charges
- We need to find how many Rb⁺ and F⁻ ions are required to create a neutral compound - The goal is to have total positive and negative charges equal to zero
Step 4:: Calculate the ratio
- Charge of Rb⁺: $$+1
- Charge of F⁻: - 1 - To balance, we need one Rb⁺ for each F⁻ - This means the ratio will be 1:1
Step 5:: Write the empirical formula
- Rubidium: $$\text{Rb}_{1}
- Fluorine: \text{F}_{1}
Final Answer
The empirical formula for the compound formed by fluorine and rubidium is RbF.
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